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Posted Date: 15 Jul 2009      Posted By:: D Shamasundar    Member Level: Gold  Points: 5 (Rs. 1)

2006 Pre University Board Education P.U.C Physics, Chemistry, Maths & Biology Karnataka 2nd PUC Chemistry Question paper Question paper



Course: P.U.C Physics, Chemistry, Maths & Biology   University/board: Pre University Board





New Scheme

Code No. 34-NS
Total No. of Questions : 39 ] [ Total No. of Printed Pages : 15
March / April, 2006

CHEMISTRY

( Kannada and English Versions )
( New Syllabus )
Time : 3 Hours ] [ Max. Marks : 90

( English Version )


Instructions : i) The question paper has four Parts.
ii) Parts A, B, C and D are common to all the candidates.
iii) Part A carries 10 marks, Each question carries one mark.
Part B carries 20 marks. Each question carries two marks.
Part C carries 40 marks. Each question carries five marks.
In Part D — D 1 carries 10 marks and D 2 carries
10 marks. Each question of D 2 carries five marks.
iv) Write balanced chemical equations and draw diagrams
wherever necessary.


PART – A

Note : i) Answer all the 10 questions.
ii) Questions have to be answered in one word or in one
sentence each. Each question carries one mark.
10 × 1 = 10
1. Out of carbon and zinc which is a stronger reducing agent ?
2. Why is Fe 3 + ion more stable than Fe 2 + ion ?
3. If the rate of the reaction is independent of concentration of the reactant,
what is the order of the reaction ?
4. Which noble gas is not adsorbed by charcoal ?
5. What is hydronium ion ?
6. What is the only factor on which the colligative property value depends ?
7. Between potassium nitrate and aluminium nitrate which one is required in
minimum concentration to coagulate arsenious sulphide sol ?
8. Which is the organic product obtained when methyl magnesium iodide
reacts with formaldehyde followed by acid hydrolysis ?
9. Name the least stable cycloalkane.
10. How many amino acid units are present in insulin ?


PART – B
Note : i) Answer any ten questions.
ii) Each question carries two marks. 10 × 2 = 20
11. Justify that concentrated sulphuric acid is a good dehydrating agent with
example.
12. Calculate the bond order in oxygen molecule.
13. The time for half-life of a first order reaction is found to be 30 mins. What
is the rate constant of the reaction ?
14. Define Faraday’s first law of electrolysis.
15. What is a spontaneous reaction ? Explain with an example.
16. What is Tyndall effect ? Explain.
17. Calculate the number of particles present in the unit cell of BCC.
11 Code No. 34-NS
36 [ Turn over
18. Distinguish between inductive effect and electromeric effect.
19. Explain the effect of the following substituents on the acidity of phenol :
i) — CH 3 group
ii) — NO 2 group.
20. How is ethanamine prepared from ethane nitrile ?
21. What are reducing and non-reducing sugars ? Give one example each.
22. What are biological messengers ? Give an example.
PART – C
I. Answer any two of the following : 2 × 5 = 10
23. a) How are noble gases separated by Dewar’s charcoal adsorption
method ? 3
b) With the help of the Ellingham’s diagram, explain why silver
oxide can be thermodynamically decomposed at relatively lower
temperature. 2
24. a) Give the postulates of Werner’s theory of coordination
compounds. 3
b) Copper (I) compounds are white and diamagnetic whereas
Copper (II) compounds are coloured and paramagnetic. Give
reason. 2
25. a) Describe the manufacture of sodium hydroxide using
Nelson’s cell. 4
b) Write the IUPAC name of ?
?
? ?
CO ( NH ) 3 4 Cl 2 Cl. 1
II. Answer any three of the following : 3 × 5 = 15
26. a) Discuss the molecular orbital structure of benzene. 3
b) Explain geometrical isomerism with an example. 2
27. a) What is S N 1 mechanism ? Explain it using hydrolysis t-butyl
bromide. 3
b) Give any two uses of aniline. 2
28. a) Write the Howarth’s ring structure for ß-D ( – ) fructopyranose.
2
b) Define the term ‘iodine value of an oil’. Mention its significance.
2
c) What is isoelectric point of amino acids ? 1
29. a) Write the equations for the following reactions : 4
i) Mixture of calcium formate and calcium benzoate is dry
distilled
ii) Acetaldehyde is treated with hydroxyl amine
iii) Acetone is treated with hydrogen cyanide
iv) Phenol is heated with a mixture of conc. nitric acid and
conc. sulphuric acid.
b) How do you convert Methane to Ethane ?


III. Answer any three of the following : 3 × 5 = 15
30. a) How are the molecular orbitals formed by the linear combination
of atomic orbitals ? 3
b) Distinguish between ideal and non-ideal solutions. 2
31. a) Calculate the mass of potassium acetate that should be
dissolved in 500 cm 3 of 0·02 M acetic acid solution to prepare
a buffer solution of pH 4·6.
Given K a = 1·8 × 10 – 5 . 3
b) Define the following terms : 2
i) Protective colloid
ii) Gold number.
32. a) Discuss the application of the principles of solubility product
with respect to the analysis of II and IV group basic radicals. 3
b) The standard free energy change ( ? G° ) for a reaction is
– 115 kJ at 27°C. Calculate the equilibrium constant ( K p ). 2
33. a) Derive an expression for the velocity constant of a first order
reaction. 4
b) Acetic acid very weakly dissociates in presence of hydrochloric
acid. Give reason. 1
34. a) With diagram, explain the construction and working of standard
hydrogen electrode. Give two limitations. 4
b) Define radius ratio in ionic crystals. 1

PART – D
D 1
IV. Answer any one of the following : 1 × 10 = 10
35. a) Explain the chemical reactions that occur during the extraction
of iron from haematite by smelting in a blast furnace. 3
b) What is angle strain ? Calculate the angle strain in cyclobutane.
3
c) What is a pseudounimolecular reaction ? Give an example. 2
d) Calculate the e.m.f. of the cell prepared by combining
Zn | 1 M ZnSO 4 and Cu | 1 M CuSO 4 at 298 K.
Given E 0
Zn = – 0·76 V and E 0
Cu = + 0·34 V . 2
36. a) On the basis of Valence bond theory, explain hybridisation,
geometrical shape and magnetic property in Cuprammonium
sulphate. 3
b) i) Explain Perkin’s reaction with an example. 2
ii) How is acetic acid prepared from ethanol ? 1
c) Calculate the osmotic pressure of 10% solution of glucose
at 27°C. Given R = 8·314 JK – 1 mol – 1 . 2
d) Give any two demerits of Arrhenius theory of ionisation. 2
15 Code No. 34-NS
36 [ Turn over
D 2
V. Answer any two of the following : 2 × 5 = 10
37. a) Explain the preparation of m-dinitrobenzene from nitrobenzene.
3
b) Describe Acrolein test. 2
38. Describe an experiment to show the effect of temperature on the rate
of the reaction between potassium persulphate and potassium
iodide. 5
39. Describe the experiment to determine the mass of Mohr’s salt
crystals in one dm 3 solution by using standard potassium
dichromate solution. Give the equation for the reaction involved. 5





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